Forming Compounds - Homework Package
SNC2D1 Grade 10 Academic Science
1. The Formation of Ions – complete the following table.
Group Example &
# of
Lose or
Bohr-Rutherford
valence
gain
diagram
electrons
electrons?
1
Li
2
Be
13
(3)
B
14
(4)
C
15
(5)
N
16
(6)
O
17
(7)
F
18
(8)
He
Ionic
charge
Name: ____________________________________________
Date: ______________________________________________
Conclusion: The atoms of the elements in each GROUP (i.e. column) share
a common property – they all have the same number of ____________________
2. What is the charge of each of the following common elements?
Element
Charge
Element
Charge
Potassium
+1
Calcium
Sulphur
Magnesium
Mercury
Bromine
Phosphorus
Barium
Iodine
Rubidium
3. Types of chemical bonds – is it ionic or molecular?
Put a checkmark () in the appropriate column.
Ionic Molecular

CaCl2
Silver bromide
CaO
Dinitrogen monoxide
CuCl2
Aluminum bromide
CO
Lead (II) oxide
Cu2O
Sodium chloride
SO2
Carbon dioxide
SnF2
Copper (II) chloride
MgCl2
dihydrogen monoxide
Li2O
Carbon monoxide
Na2O
Zinc oxide
PbI2
Aluminum oxide
CO2
Copper (II) oxide
FeCl2
Calcium chloride
NaCl
Potassium chloride
SO3
Tin (II) chloride
NaI
Nitrogen dioxide
KCl
Sodium fluoride
PbCl2
Sulphur trioxide
K2O
Lithium oxide
N2O5
Zinc chloride
Ionic
Molecular
IONIC BONDING
Ionic bonding occurs when a ________________ and transfers one or more
electrons to a _______________ in an effort to attain a stable ___________ of
electrons.
1. Show the transfer of electrons using Bohr-Rutherford diagrams in
the following combinations.
K+F
For example, the transfer of one electron from a sodium to chlorine atom
can be depicted by the Bohr-Rutherford diagram below:
Mg + I
The attraction between the newly formed cation and anion is called the
ionic bond.
Be + S
Example 2: Al and Cl
Aluminum would need three chlorine
atoms to get rid of its 3 valence
electrons.
The concept:
The total positive charge and the total
negative charge needs to equal ZERO in
order to form a stable ionic compound.
So…Al3+ is a stable cation, and Cl- is a
stable anion. But there are more
positive charges than negative charges if
there is only one of each. So there needs
to be a total of 3 negative charges to
balance out the 3 positive charges that
Al3+ has. Therefore, three chlorine ions
are needed for every aluminum ion
present.
Na + O
Al + Br
Forming Ionic Compounds
Anion
Chemical Formula
Name of Compound
Cation
Cation
Anion
Cation
Anion
Cation
Anion
Cation
Anion
Chemical Formula
I-
Li1 I1
LiI
Lithium iodide
Crisscross
Anion
Crisscross
Li+
Lithium + Iodine
Cation
Potassium + Fluorine
2. Complete the following tables:
Example 1:
Elements
Cation
Elements
Elements
Anion
Calcium + Bromine
Name of Compound
Elements
Beryllium + oxygen
Crisscross
Chemical Formula
Name of Compound
Crisscross
Chemical Formula
Elements
Name of Compound
Calcium + nitrogen
Crisscross
Elements
Cation
Anion
Aluminum + Chlorine
Chemical Formula
Name of Compound
Crisscross
Chemical Formula
Elements
Name of Compound
Magnesium + phosphorus
Crisscross
Elements
Magnesium + Sulphur
Cation
Anion
Chemical Formula
Name of Compound
Crisscross
Chemical Formula
Elements
Name of Compound
Aluminum + oxygen
Crisscross
Chemical Formula
Name of Compound
Elements with Multiple Ionic Charges
1. Complete the following tables.
Example 1:
Name of Compound
Cation
Tin (II) iodide
Sn2+
ISn1 I2
SnI2
Crisscross
Chemical Formula
Name of Compound
Anion
Cation
Anion
Copper (I) bromide
Crisscross
Chemical Formula
Name of Compound
Cation
Anion
Cation
Anion
Cation
Anion
Iron (III) chloride
Crisscross
Chemical Formula
Name of Compound
Tin(IV) fluoride
Crisscross
Chemical Formula
Name of Compound
Iron (II) oxide
Crisscross
Chemical Formula
2. Write the chemical names for the following compounds.
a. CuCl2
Copper (II) chloride
b. FeBr3
c. PbS
d. SnO2
e. FeP
f. CuI
g. PbI2
h. FeCl2
i. SnF2
j. PbCl2
k. Cu2O
3. More practice!
PART A: Write the chemical formula for the following compounds
a. Copper (II) oxide
b. Silver chloride
c. Tin (II) chloride
d. Cobalt (II) phosphide
e. Sodium fluoride
f. Lithium oxide
g. Lead (II) oxide
h. Iron (III) oxide
i. Magnesium bromide
j. Zinc oxide
k. Chromium (II) bromide
l. Nickel (III) oxide
m. Lead (IV) oxide
n. Aluminum nitride
o. Lithium iodide
p. Copper (II) chloride
PART B: Write the chemical names for the following compounds
a. NaCl
b. MgCl2
c. FeCl3
d. FeO
e. Mg3N2
f. Cu3N
g. SnS2
h. AuCl3
i. Fe2O3
j. Cu3P2
k. CuF2
l. LiBr
m. K3P
Polyatomic Ions
1. Complete the following tables.
Example 1:
Name of Compound
Cation
Na+
Sodium phosphate
Crisscross
Chemical Formula
Name of Compound
Anion
(PO4)3Na3 (PO4)1
Na3PO4
Cation
Anion
Cation
Anion
Calcium sulphate
Crisscross
Chemical Formula
Name of Compound
Copper (I) carbonate
Crisscross
Chemical Formula
Name of Compound
Cation
Anion
Cation
Anion
Tin (II) hydroxide
Crisscross
Chemical Formula
Name of Compound
Sodium chlorate
Crisscross
Chemical Formula
2.
a.
b.
c.
d.
e.
f.
g.
h.
Write the chemical names for the following compounds.
KNO3 (found in gun powder)
Potassium nitrate
Ca(OH)2 (an ingredient in plaster)
CaCO3 (in chalk)
CuSO4 (a fungicide)
KOH (used to make soap)
Fe(NO3)3 (used in water treatment)
Cu(ClO3)2 (used to colour fireworks)
(NH4)3PO4 (ingredient in bread dough)
3.
a.
b.
c.
d.
e.
f.
g.
h.
Write the chemical formula for each of the following compounds.
Potassium nitrate (used to colour fireworks purple)
Barium sulphate (given prior to an X-ray of the intestine)
Ammonium nitrate (common ingredient in fertilizer)
Aluminum sulphate (used in preparing pickles)
Potassium chlorate (an explosive)
Copper (II) nitrate (used to colour ceramics)
Lead (II) sulphate (found in car batteries)
Tin (II) phosphate (used in the dyeing of silk)
4. More Practice!
PART A: Write the chemical names for the following compounds.
a. Li2CO3
b. Mg3(PO4)2
c. K2SO4
d. NaNO3
e. Al(OH)3
f. Pb3(PO4)2
g. Sn(ClO3)2
h. NaOH
i. FeSO4
j. K3PO4
PART B: Write the chemical formulas for the following compounds.
a.
c.
e.
g.
i.
k.
m.
Magnesium sulphate
Sodium chlorate
Aluminum nitrate
Sodium bicarbonate
Copper (II) hydroxide
Iron (II) phosphate
Beryllium sulphate
b.
d.
f.
h.
j.
l.
n.
Copper (I) chlorate
Magnesium hydroxide
Lead (II) nitrate
Aluminum carbonate
Ammonium sulphate
Cobalt (II) phosphate
Barium nitrate
Ionic Compounds – Review
Write the chemical formulas and chemical names of the compounds produced from the listed ion in the grid below.
Cl-
Na+
NH4+
K+
Ca2+
Mg2+
Zn2+
Fe2+
Al3+
Co3+
Fe3+
H+
Example:
NaCl
Sodium
chloride
CO32-
OH-
SO42-
PO43-
NO3-
Molecular compounds - Covalent bonds
Covalent bonding occurs when two more __________________ SHARE electrons,
attempting to attain a stable octet of electrons at least part of the time.
(Note: Hydrogen is stable with 2 electrons, not 8!)
1. Using Bohr-Rutherford diagrams, show how covalent bonding occurs in
each of the following pairs of atoms.
Atoms may share one, two, or three pairs of electrons (i.e. there can be a
single bond, double bond, or triple bond between atoms).
a. H + H (H2)
b. F + F (F2)
c. O + O (O2)
d. N + N (N2)
e. C + O (CO2)
f.
H + O (H2O)
Naming molecular compounds using the prefix method:
1*
2
3
4
5
Prefix
mono*MONO is only
used with the
2nd non-metal!
2. Write the chemical formula for the following molecular compounds.
a. Carbon dioxide
CO2
b. Silicon dioxide
c. Carbon disulfide
d. Sulphur trioxide
e. Carbon tetrachloride
f. Diphosphorus trioxide
g. Dinitrogen oxide
h. Arsenic tribromide
i. Phosphorus pentrabromide
j. Dinitrogen tetroxide
k. Silicon carbide
l. Sulphur dioxide
m. Dinitrogen monoxide
n. Sulphur difluoride
3. Write the chemical name for the following molecular compounds.
a. CF4
Carbon tetrafluoride
b. PBr3
c. CS2
d. N2O2
e. H2O2
f. CO
g. N2O3
h. SiC
i. P2O5
j. SO3
k. SiO2
l. PCl5
m. N2O5
4. Ionic or Covalent
For each of the following compounds, place a checkmark () under the
appropriate column to state if it is IONIC or COVALENT and name the
compound.
Compound
Example: BaS
a. Rb3N
b. N2S5
c. BeO
d. HI
e. SrCl2
f.
FeCl3
g. P2S5
h. SCl2
i.
Ag(NO3)
j.
As2S3
k. Cu(HCO3)2
l.
SnO2
m. K3(PO4)
n. NaCl
o. CCl4
Ionic Covalent

Chemical Name
Barium sulphide
Naming & writing chemical formulas for
ionic & molecular compounds.
5. Write the chemical formula for the following compounds.
Lithium bromide
Carbon monoxide
Arsenic trifluoride
Mercury (II) sulfate
Barium hydride
Cobalt (III) chloride
Calcium phosphate
Phosphorus pentachloride
Tin (IV) iodide
Copper (I) oxide
Sodium sulfide
Dinitrogen trisulfide
Iodine monobromide
Beryllium bromide
Lead (II) carbonate
Lead (IV) oxide
Selenium tribromide
Potassium chlorate
Barium nitrate
Chromium (II) nitrate
Ammonium sulfide
Calcium bicarbonate
Barium iodate
Manganese (II) fluoride
Sodium hydroxide
Calcium hydroxide
Ammonium sulfate
Tricarbon tetraphosphide
Chromium (III) oxide
Iron (III) carbonate
Hydrogen sulfide
Magnesium nitride
p. NO
2. Write the correct name for each of the following compounds
NF3
Ag3N
q. Na2(SO4)
K2SO4
CrCl3
r.
Na3P
Au2O3
s. CO2
Co(NO3)3
KOH
t.
Fe2S3
Co(ClO3)2
u. BaSO4
P2S5
Li(NO3)
v. K2O
Ca3(PO4)2
Mg3(PO4)2
w. NaF
CBr4
Si3N2
x. Na2CO3
SO2
Fe(ClO3)2
CaCl2
H2O
y. NH4Cl